The first ionization potential (eV) of N and P respectively are

Options

A. `8.29, 8.29`
B. `11.32 , 11.32`
C. `8.29 , 11.32`
D. `11.32, 8.21`

Answer

To determine the first ionization potential (IP) of nitrogen (N) and phosphorus (P), we need to understand the trends in ionization energy across the periodic table.

### Step-by-Step Solution:

1. **Understanding Ionization Potential**:
- Ionization potential (or ionization energy) is the energy required to remove an electron from an atom in its gaseous state.

2. **Periodic Trends**:
- Ionization energy generally increases from left to right across a period due to increasing nuclear charge.
- Ionization energy generally decreases down a group due to increased distance of the outer electrons from the nucleus and increased shielding effect.

3. **Position of Nitrogen and Phosphorus**:
- Nitrogen (N) is located in Group 15 (or Group V) and Period 2.
- Phosphorus (P) is located in Group 15 (or Group V) and Period 3.

4. **Comparing Ionization Energies**:
- As we move from nitrogen (Period 2) to phosphorus (Period 3), we expect the ionization energy to decrease due to the reasons mentioned above (increased distance and shielding).

5. **Values of Ionization Potentials**:
- The first ionization potential of nitrogen (N) is approximately **11.32 eV**.
- The first ionization potential of phosphorus (P) is approximately **8.21 eV**.

6. **Conclusion**:
- Therefore, the first ionization potentials of nitrogen and phosphorus are **11.32 eV** and **8.21 eV**, respectively.

### Final Answer:
The first ionization potential of N and P are **11.32 eV** and **8.21 eV** respectively.

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